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defon
2 years ago
11

Four students wrote different analogies to describe an electron before the formation of an ionic bond . Student A: A tug of war

between two wrestlers each weighing 460 lbs Student B: A dog and his owner tugging at a frisbee Student A big greedy dog stealing away a bone from a smaller dog Student D: Children exchanging their orange and strawberry flavored popsicles Which student presented a correct analogy ?
Chemistry
1 answer:
Nutka1998 [239]2 years ago
3 0

The correct analogy is that of "A big greedy dog stealing away a bone from a smaller dog."

An ionic bond is a bond formed formed between a metallic atom and a non-metallic atom.

The metallic atom is electropositive while the non-metallic atom is electronegative. Therefore, the metallic atom donates or gives up its electrons to the non-metallic atom which accepts the electrons.

During the formation of chemical bonds, only valence or outermost shell electrons are involved.

Metallic atoms have few valence electrons (between 1 to 3 electrons) while non-metallic atoms have many valence electrons (between 5 to 7 electrons).

Therefore the analogy by the student of a big greedy dog stealing away a bone from a smaller dog is correct because the non-metallic atoms takes the few electrons of the metallic atom and add to the many electrons they already have during the formation of an ionic bond.

Learn more about an ionic bond at: brainly.com/question/1225796

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The average rate of consumption of br− is 1.86×10−4 m/s over the first two minutes. what is the average rate of formation of br2
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3 years ago
What mass in grams would 5.7L of hydrogen gas occupy at STP?​
tekilochka [14]

Answer:  The correct answer is:  " 0.54 g " .

__________________________________________

Explanation:

Note that "hydrogen gas" is:  

H₂ (g)  ;   that is:  a "diatomic element" (diatomic gas) ;

_________________________________________

The molecular weight of "H" is:  1.00794 g ;

   (From the Periodic Table of Elements).

So, the molecular weight of:  H₂ (g)  is:

    " 1.00794 g * 2  = 2.01588 g ; {use calculator) ;

_________________________________________

Note the conversion for a gas at STP:

______

  1 mol of a gas = 22.4 L gas;

___

i.e. " 1 mol / 22.4 L " ;

____

So:     " 5.7 L H₂ (g)  *  \frac{1 mol H_{2} }{22.4 L} *\frac{2.01588 g}{mol} =? ;

The "L" ("literes" cancel out to "1" ;  since "L/L = 1 ;

The "mol" (moles) cancel out to "1" ; since "mol/mol = 1 ;

____

and we are left with:

____

 [5.7 * 2.104588 g ] / 22.4  =  ?  g ;

______________________

→ [ 11.9961516  g ] / 22.4 =

          0.53554248214  g ;l

_____________________________

We round this value to:  " 0.54 g " ;

 → since "5.7 L " has 2 (two) significant figures;  

     22.4 is an exact number conversion;

     and "5.7 L" has fewer significant figures than:

    " 2.104588 " ; or:  " 1.00794 " .

  → as such: We round to "2 (two) significant figures."

______________________________

Hope this is helpful.  Wishing you the best in your academic endeavors!

_______________________________

8 0
3 years ago
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